H2 and I2 react in an exothermic reaction according to the following equation: H2 (g) + I2 (g) Double arrow yields 2HI (g) H2 and I2 are placed in a sealed container and are allowed to reach equilibrium. What could you change about the system that would shift its equilibrium position? Add a catalyst. Decrease the volume. Increase the pressure. Lower the temperature.

Question

Xander Odom

Chemistry

24 January, 18:15

H2 and I2 react in an exothermic reaction according to the following equation: H2 (g) + I2 (g) Double arrow yields 2HI (g) H2 and I2 are placed in a sealed container and are allowed to reach equilibrium. What could you change about the system that would shift its equilibrium position? Add a catalyst. Decrease the volume. Increase the pressure. Lower the temperature.

+2

Answers (1)

Know the Answer?

Deandre Travis · Answer 1

Adding a catalyst would not change the equilibrium because it keeps the rates of forward and reverse the same.

Increasing the pressure wouldn't affect it because on both sides, there are the same number of moles.

It's either temperature or volume.